Which of the following substances have permanent dipole-dipole forces? (a) GeH4 ; (b) molecular

step 1 In this question we've been given some molecules and asked to determine which ones have got perm

Which of the following substances have permanent...

Key Concepts

Intermolecular Forces

Intermolecular forces are attractions between molecules that determine many of a substance's physical properties. They include various types such as London dispersion forces, permanent dipole–dipole interactions, and hydrogen bonding. Understanding these forces helps in predicting boiling points, melting points, and solubilities.

Permanent Dipole–Dipole Interactions

Permanent dipole–dipole interactions arise when polar molecules, which have a permanent separation of charge, attract each other. These forces occur when the positive end of one polar molecule is attracted to the negative end of another. They are stronger than dispersion forces but generally weaker than hydrogen bonds.

Molecular Polarity

Molecular polarity refers to the existence of a net dipole moment in a molecule, caused by differences in electronegativity between bonded atoms and the molecule's three?dimensional shape. A molecule is polar if the individual bond dipoles do not cancel out due to asymmetry in its geometry, thereby giving rise to permanent dipole–dipole interactions.

Molecular Geometry

Molecular geometry is the three-dimensional arrangement of atoms within a molecule. The geometry determines whether individual bond dipoles cancel out or add up to create a net dipole moment. Symmetrical molecules often have no net dipole moment, even if the bonds themselves are polar, while asymmetrical molecules are typically polar and exhibit permanent dipole–dipole forces.

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